Patterns in the periodic table
Use G2 Science Chemistry electron arrangements to explain periodic groups, compare metal reactivity and understand how barrier coatings prevent rusting.
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Before you begin
Use G2 Science Chemistry electron arrangements to explain periodic groups, compare metal reactivity and understand how barrier coatings prevent rusting.
Learning goals
- Describe the Periodic Table as the elements arranged in order of increasing proton number
- Relate an element's position in the Periodic Table to its proton number and electronic configuration
- Explain why elements in the same group are similar using their electronic configurations
- Describe the change from metallic to non-metallic character across a period
- Relate the number of outer (valence) electrons to metallic or non-metallic character
- Predict the properties of Group 1 and Group 17 elements from the Periodic Table
- Describe lithium, sodium and potassium as soft, low-density metals with trends in melting point and reaction with water
- Describe chlorine, bromine and iodine as diatomic non-metals with trends in colour, state and displacement of other halide ions
- Explain why Group 18 elements are unreactive using their electronic configurations
- Place common metals and hydrogen in order of reactivity from their reactions with water, steam and dilute hydrochloric acid
- Deduce an order of reactivity from experimental results
- Relate how easily a metal is extracted from its ore to its position in the reactivity series
- Describe the conditions needed for iron to rust and how a barrier, such as paint, grease or plastic, prevents it
Syllabus statements covered
- describe the Periodic Table as an arrangement of the elements in the order of increasing proton (atomic) number
- describe how the position of an element in the Periodic Table is related to proton number and electronic configuration
- explain the similarities between the elements in the same group of the Periodic Table in terms of their electronic configuration
- describe the change from metallic to non-metallic character from left to right across a period of the Periodic Table
- describe the relationship between number of outer (valence) electrons and metallic/non-metallic character
- predict the properties of elements in Group 1 and Group 17 using the Periodic Table.
- describe lithium, sodium and potassium in Group 1 (the alkali metals) as a collection of relatively soft, low density metals showing a trend in melting point and in their reaction with water
- describe chlorine, bromine and iodine in Group 17 (the halogens) as a collection of diatomic non- metals showing a trend in colour, state and their displacement reactions with solutions of other halide ions
- describe the lack of reactivity of the elements in Group 18 (the noble gases) in terms of their electronic configurations.
- place in order of reactivity calcium, copper, (hydrogen), iron, lead, magnesium, potassium, silver, sodium and zinc by reference to the reactions, if any, of the metals with water, steam and dilute hydrochloric acid
- deduce the order of reactivity from a given set of experimental results
- describe the ease of obtaining metals from their ores by relating the elements to their positions in the reactivity series
- describe the essential conditions for the corrosion (rusting) of iron as the presence of oxygen and water; prevention of rusting can be achieved by placing a barrier around the metal, e.g. painting; greasing; plastic coating.
Lessons
Work through them in order.
- Periodic table position and patternsPlace an element from its proton number and electron arrangement, and predict whether it behaves as a metal or a non-metal.
- Group 1: reactions and trendsUse water reactions and physical data to explain and predict Group 1 trends.
- Group 17: halogens and displacementPredict halogen displacement and connect reactivity to electron gain.
- Group 18: noble gases and group comparisonsExplain why noble gases are unreactive, then compare the three group patterns.
- The reactivity series and obtaining metalsOrder metals from reaction results, spot results that cannot decide an order, and relate reactivity to how easily a metal is obtained.
- Rusting and preventing itShow from a controlled experiment that rusting needs oxygen and water, and explain how a barrier stops it.
Practise and check
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